Can you store `CuSO_(4)` solution in `Zn` pot ?

Explanation

Since the standard reduction potential of Zn is less than that of copper, hence zinc metal will reduce `Cu^(2+)` ions present in aqueous solution of copper sulphate. Thus, we can not store copper sulphate solution in a vessel of zinc.
`Zn(s)+CuSO_(4)(aq)hArrZnSO_(4)(aq)+Cu`
`E_("Redox process")^(0)=E_("Reducedspecies")^(0)-E_("Oxidisedspecies")^(0)`
`=+0.34-(-0.76)=+1.10V`
Positive value of `E^(@)` confirms that above redox process is spontaneous and hence we cannot store copper sulphate solution in a vessel of zinc.